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For one mole of an ideal gas, increasing the temperature from 10°C to 20°C ______.
With increase of pressure, the mean free path:
At what temperature the RMS velocity of SO_{2} be same as that of O_{2} at 303 K
An ideal gas obeying kinetic theory of gases can be liquefied if:
For the process
H_{2}O(l) → H_{2}O(g)
At T = 100°C and 1 atmosphere pressure, the correct choice is:
One mole of a monoatomic ideal gas expands adiabatically at initial temperature T against a constant external pressure of 1 atm from 1L to 3L. The final temperature of the gas is:
The enthalpies of combustion of carbon and carbon monoxide are –393.5 and –283 kJ mol^{–1}, respectively. The enthalpy of formation of carbon monoxide per mole is:
The Maxwell's relationship derived from the equation dG = VdP – SdT is:
For a closed system consisting of a reaction N_{2}O_{4}(g) → 2NO_{2}(g), the pressure:
One mole of an ideal gas is put through a series of changes as shown in the graph in which A, B, C mark the three stages of system. Calculate the pressure at three stages of the system & provide the sum value (P_{A} + P_{B} + P_{C})
If at 298 K the bond energies of C—H, C—C, C=C and H—H are, respectively, 414, 347, 615 and 435 kJ mol^{–1}, the value of enthalpy change for the reaction CH_{2}=CH_{2}(g) + H_{2}(g) → H_{3}C—CH_{3}(g) at 298 K will be:
2 mole 'He' is mixed with 2gm of H_{2}. The molar heat capacity at constant pressure for mixture is:
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If T_{i} is the initial temperature and T_{f} is the final temperature, which of the following statement is correct:
An inventor claims to have constructed an engine that has an efficiency of 75% when operated between the boiling and freezing points of water. Which of the following is true?
If C_{1}, C_{2}, C_{3}........ represent the speeds of n_{1}, n_{2}, n_{3}....... molecules, then the root mean square speed is:
A bubble of air is underwater at temperature 15°C and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is 25°C and the pressure is 1.0 bar, what will happen to the volume of the bubble?
0.5 mole of each of H_{2}, SO_{2} and CH_{4} are kept in a container. A hole was made in the container. After 3 hours, the order of partial pressures in the container will be:
Volume of air that will be expelled from a vessel of 300 cm^{3} when it is heated from 27^{o}C o 37^{o}C at the same pressure will be
Two separate bulbs contain ideal gases A and B. The density of gas A is twice that of gas B. The molecular mass of A is half that of gas B. The two gases are at the same temperature. The ratio of the pressure of A to that of gas B is:
The molar entropy of crystalline CO at absolute zero is:
The plot that describes a Carnot cycle is:
The rate of evaporation of a liquid is always faster at a higher temperature because:
For the process,
1 Ar (300 K, 1 bar) → 1Ar (200 K, 10 bar) assuming ideal gas behaviour, the change in molar entropy is:
For the reaction, N_{2}(g) + 3H_{2}(g) → 2NH_{3}(g)
Compute the entropy change (in J/K/mol) for the process and comment on the sign of the property.
For the reaction,
2Cl(g) → Cl_{2}(g)
The thermodynamic properties
The standard enthalpies of formation of CO_{2}(g), H_{2}O(l) and glucose(s) at 25°C are –400 kJ mol^{–1},
–300 kJ mol^{–1} and –1300 kJ mol^{–1}, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is:
For an ideal gas, which of the following is true:
Assuming that water vapour is an ideal gas, the internal energy change (∆U) when 1 mol of water is vaporized at 1 bar pressure and 100°C will be (given that molar enthalpy of vaporisation of water at 1 bar and 373 K is 41 kJ mol^{–1} K^{–1})
For a system of constant composition, the pressure (P) is given by:
Identify the intensive quantities from the following:
Among the following which are/is state function(s):
Select the correct statements for ideal gases:
The incorrect expression among the following is:
Indicate which one of the following relations is not correct:
The species which by definition has zero standard molar enthalpy of formation at 298 K is:
An ideal gas obeying kinetic theory of gases can be liquefied if:
Sponteneous adsorption of a gas on solid surface is an exothermic process because
Indicate the correct statement for a 1L sample of N_{2}(g) and CO_{2}(g) at 298 K and 1 atm pressure:
A gas expands against a variable external pressure given by p = 10/V atm, where V is the volume at each stage of expansion. In expanding from 10 L to 100 L, the gas undergoes a change in internal energy ∆U = 418 J. How much heat (kJ) has been absorbed? [rounded up to two decimal places]
Calculate the work done (J) when 1 mole of zinc dissolves in hydrochloric acid at 273 K in a closed beaker at 300 K [Volume at STP = 22.4 L, rounded up to two decimal places]:
Calculate the enthalpy change (calmol^{–1}) when 36 g of water is heated from 27°C to 37°C at 1 atm pressure. The molar heat capacity of water (18.1 cal K^{–1}mol^{–1}) remains constant in this temperature range: [rounded up to two decimal places]
Given the following thermo chemical equations:
Calculate ∆H°(kJ mol^{–1}) for this reaction: N_{2}O(g) + 1/2 O_{2}(g) → 2NO(g) [rounded up to two decimal places]
Acetone, the solvent usually found in nail polish remover and has the structural formula
Approximately how much energy (kJ) would be released during the formation of the bonds in one mole of acetone molecules? [In the multiple of 10^{3}, rounded up to two decimal places]
Given: C—H = 412 kJ/mol; C—C = 348; C=O = 743.
Diborane is a potential rocket fuel which undergoes combustion according to the reaction,
From the follwoing data, calculate the enthalpy change (kJ mol^{–1)} for the combustion of diborane:
A gas is found to have a formula [CO]_{x}. If its vapor density is 70, the value of x is:
2g of gas X are introduced into an evacuated flask kept at 25^{o}C. The pressure is found to be 1atm. If 3g of another gas ‘Y’ are added to same flask, the total pressure becomes 1.5 atm. Assuming that ideal behavior, the molecular mass ratio of M_{x} and M_{y} is:
The density of a gas at 27°C and 1 atm is d. Pressure remaining constant at which temperature(K) will its density become 0.75 d: [rounded up to two decimal places]
Pressure exerted by 1 mole of methane in a 0.25 litre container at 300 K using van der Waal's equation (given a = 2.253 atml^{2}mol^{–2}, b = 0.0428 litmol^{–1}) is (in atm): [rounded up to two decimal places]
Find the maximum work done (cal) when 0.5 mol of a gas expands isothermally and reversibly from a volume of 2L to 5L at 27°C and calculate the change in internal energy if 200 cal of heat is absrobed? [rounded up to two decimal places]
For the following reaction
∆H = 40 kJ/mol
C_{p}(H_{2}O, l) = 40 J/mol K
C_{p}(H_{2}O, g) = 30 J/mol K
Then calculate ∆G(J/mol) at 1 atm, 373 K:
For the reaction,
2CO + O_{2} → 2CO_{2}; ΔH = 560KJ
Two moles of CO and one mole of O_{2} are taken in a container of volume 1L. They completely form two moles of CO_{2}, the gases deviated appreciably from ideal behavior. If the pressure in the vessel changes from 70 to 40 atm, find the magnitude (kJ) of ∆U at 500 K. (1L atm = 0.1 kJ) [rounded up to two decimal places]
If 22 g of CO_{2}, showing ideal behaviour, isothermally and reversibly from 2.5 L to 7.5 L at 27°C, then calculate the work done (J) and heat absorbed: [rounded up to two decimal places]
One mole of an ideal gas is subjected to a change from 10 atm to 1 atm at 300 K. Calculate (in JK^{1} rounded up to three decimal places) ∆S_{surrounding} = ? [R = 8.314 JK^{1}mol^{1]}
What is the boiling point(°C) of a liquid with entropy of vaporization 68.3 JK^{–1}mol^{–1} and enthalpy of vaporization 35.65 kJ mol^{–1}: [rounded up to two decimal places]
2 mol of an ideal gas expanded isothermally and reversibly from 1L to 10L at 300 K. What is the enthalpy change(kJ)?
Containers A and B have same gases. Pressure, volume and temperature of A are all twice that of B, then the ratio of number of molecules of A and B are:
At identical temp and pressure the rate of diffusion of hydrogen gas is 5.19 times that of hydrocarbon having molecular formula C_{n}H_{2n2}. What is value of ‘n’ ?
For one mole of a Vander Waals gas when b = 0 and T = 300 K, the PV vs 1/V plot is shown below. The value of the van der Waals constant a (atm. litre^{2}mol^{–2}) is: [rounded up to first decimal place]
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